Mercury(II) nitrate

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Mercury(II) nitrate
Mercury nitrate.png
Names
IUPAC names
Mercury dinitrate
Mercury(II) nitrate
Other names
Mercuric nitrate
Identifiers
10045-94-0 N
7783-34-8 (monohydrate) N
EC number 233-152-3
PubChem 24864
RTECS number OW8225000
UN number 1625
Properties
Hg(NO3)2
Molar mass 324.60 g/mol (anhydrous)
Appearance colorless crystals or white powder
Odor sharp
Density 4.3 g/cm3 (monohydrate)
Melting point 79 °C (174 °F; 352 K) (monohydrate)
soluble
Solubility soluble in nitric acid, acetone, ammonia
insoluble in alcohol
Hazards
Safety data sheet ICSC 0980
EU classification Very toxic (T+)
Dangerous for the environment (N)
R-phrases R26/27/28, R33, R50/53
S-phrases (S1/2), S13, S28, S45, S60, S61
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Flash point Non-flammable
Related compounds
Other anions
Mercury(II) sulfate
Mercury(II) chloride
Other cations
Zinc nitrate
Cadmium nitrate
Related compounds
Mercury(I) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Mercury(II) nitrate is a toxic colorless or white soluble crystalline mercury(II) salt of nitric acid. It was also used to treat fur to make felt in a process called 'carroting'. The phrase 'mad as a hatter' is associated with psychological illness brought on by excessive exposure to mercury(II) nitrate. The practice continued in the United States until it was banned in December 1941 by the United States Public Health Service. Although this sounds beneficial to health, the ban actually freed mercury(II)nitrate to be used as a detonator in the then ongoing war.[1]

Production[edit]

It is made by reacting hot concentrated nitric acid with mercury metal, it is an oxidizing agent. Dilute nitric acid would produce mercury(I) nitrate.

Uses[edit]

Mercuric acid is used in mercuration reactions. In particular, it is used in reactions involving ketones. One of the chemicals which it is most effective with is acetone. This reaction uses mercuric nitrate, mercuric oxide, and calcium sulfate to change acetone, which is CH3C(O)CH3, into CH3C(O)CH2HgI. Acetone is a compound for which most other methods of mercuration prove ineffective.[2] The mercuric nitrate compound works because it is a strong oxidizing agent.[3] In addition, when mercury is dissolved in nitric acid the acid form of mercuric nitrate is formed.[4] The acidic form is capable of inverting molecules of sucrose.[5]

Health Information[edit]

Mercury nitrate tends to impact the body as Hg2+, which is considered a form of inorganic mercury. Forms an inorganic mercury can be found in various contexts including in skin lightening cream. If the inorganic mercury is ingested it can change the structure of important proteins within the body If it gets into the soil it can then be absorbed and remain to be taken up by plants.[6] Those suffering from poisoning tend to experience vomiting and diarrhea as their earliest symptoms.[3]

Reactivity[edit]

Although mercuric nitrate is not flammable it can speed up flames since it acts as an oxidizer. In addition, it can form explosive compounds when combined with alcohols.[7]

See also[edit]

References[edit]

  1. ^ "The Not-So-Mad Hatter: Occupational Hazards of Mercury". 
  2. ^ "Mercuration of Ketones and Some Other Compounds with Mercuric Nitrate". 
  3. ^ a b "Mercuric Nitrate". 
  4. ^ "Foods:Their Compostition and Analysis". 
  5. ^ "The Inversion of Sucrosse by Acid Mercuric Nitrate". 
  6. ^ "Elemental Mercury and Inorganic Mercury Compounds:Human Health Aspects" (PDF). 
  7. ^ "Mercuric Nitrate". 

External links[edit]

Salts and covalent derivatives of the Nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)4 C N O FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)3 Co(NO3)2,
Co(NO3)3
Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I Xe
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Hg(NO3)2
Tl(NO3)3 Pb(NO3)2 Bi(NO3)3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
La Ce(NO3)3,
Ce(NO3)4
Pr Nd Pm Sm Eu Gd(NO3)3 Tb Dy Ho Er Tm Yb Lu
Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr